Nitric acid is a strong oxidizing agent that is colorless and highly corrosive. It is produced industrially via the Ostwald process, which involves the oxidation of ammonia to nitric oxide using a platinum catalyst and air, followed by the oxidation of nitric oxide to nitrogen dioxide and its absorption in water to form nitric acid. Nitric acid has a variety of uses including as a fertilizer component and nitrating agent for explosives. Hydrochloric acid is also a strong corrosive acid that is produced from chlorination byproducts or by reacting metallic chlorides with sulfuric acid. It is used in a variety of industrial processes.
3. Introduction
Nitric acid is a strong mineral acid. It is a mono-basic acid.
It is a strong oxidizing agent and can oxidize metals and
nonmetals easily.
Nitric acid (HNO3) is a colorless liquid that is used in the
manufacture of inorganic and organic nitrates and nitro
compounds for fertilizers, dye intermediates, explosives, and
many different organic chemicals.
4. Properties
HNO3 is usually a fuming liquid.
It is freely miscible with water.
It freezes to a snow white solid at -46 C.
It is a colorless volatile liquid.
It has a pungent smell.
Its specific gravity at 15 C is 1.53.
5. Uses
As a starting material in the manufacture of nitrogen
fertilizers such as ammonium nitrate & ammonium etc. Large
amounts are reacted with ammonia to yield ammonium
nitrate.
As a nitrating agent in the preparation of explosives such as
TNT, ammonium picrate (Dunnite)
It is commonly used in science laboratories at schools for
experimenting when specifically testing for chloride.
7. Methods
INDUSTRIALLY NITRIC ACID IS PREPARED BY
FOLLOWING 3 METHODS:
CHILE SALTPETRE METHOD BY NANO3
BRIKLAND EYDE’S METHOD BY USING AIR
OSTWALD’S METHOD
8. OSTWALD’S METHOD
Principle
NH3 is oxidized into NO by air at 800 C in presence of Pt
(Platinum)catalyst with 10% Rh content.
Materials used:
Ammonia gas
Water
Oxygen gas
9. PROCESS
The conversion of ammonia into nitric acid in this process is
done through the following steps:
Step1
Oxidation of ammonia to nitric oxide
Ammonia is oxidized by air in the presence of Pt catalyst at
800°C to give nitric oxide.
4NH3 + 5O2 ——–> 4NO + 6H2O
Heat liberated maintains the temperature of the catalyst.
10. Cont.
Step 2
Oxidation of NO to NO2
The nitric oxide is oxidized by air at temperature below
100°C, to give nitrogen dioxide (NO2)
2NO + O2 ——> 2NO2
11. Cont.
Step 3
Formation of nitric acid
Nitrogen dioxide is then converted to nitric acid by absorbing
NO2 in water, in the presence of air.
3NO2 + H2O ——> 2HNO3 + NO
14. Introduction
Hydrochloric acid is a clear, colorless, highly pungent solution of
hydrogen chloride (HCl) in water.
It is a highly corrosive, strong mineral acid with many industrial
uses. Hydrochloric acid is found naturally in gastric acid.
As an monoprotic acid and one of the six common strong
mineral acids, it is the least likely to be subject to an oxidation-
reduction reaction.
15. Properties
It is available in many different concentrations in water, thus
its exact physical properties (boiling point, melting point and
density) vary accordingly.
The concentrated grade (fuming hydrochloric acid) is about
38% HCl in water.
Industrial-grade HCl is about 30% to 35%, while the
commercial grade (muriatic acid) is between 20% and 32%.
Household cleaning solutions of HCl are typically 10% to
12%, but these still need further dilution before use.
17. Methods
Synthesis from elements (Burning Process)
Organic By-product Synthesis.
Metallic chlorides with Sulfuric acid.
Waste Incineration.
Thermal decomposition of hydrated heavy metals
18. Organic by-product Synthesis
Hydrochloric acid is made during chlorination of organic products as
follows:
RH₂+ Cl₂→RCl + HCl
Hydrochloric acid is also made during fluorination of chlorinated organic
products to manufacture (hydro)chlorofluorocarbons as follows:
RCl + HF →RF + HCl
Where RCl stands for chloroform, trichloro ethane, etc and RF
stands for (hydro) chlorofluorocarbons
19.
20. Waste Incineration.
From incineration of chlorinated organic waste:
C4H6Cl2 + 5O2 → 4CO2 + 2H2O + 2HCl
After leaving the chlorination process, the HCl-containing gas
stream proceeds to the absorption column, where concentrated
liquid HCl is produced by absorption of HCl vapors into a weak
solution of hydrochloric acid.
The HCl-free chlorination gases are removed for further
processing. The liquid acid is then either sold or used elsewhere
in the plant. The final gas stream is sent to a scrubber to remove
the remaining HCl prior to venting.